A 10.0-mL sample of sulfuric acid, H2SO4, from a battery of an old car is diluted to 100.0 mL, and a 10.00-mL aliquot (portion) of the diluted acid is then titrated with 0.2500 M NaOH solution. If the concentration of H2SO4 in the original battery was 3.25 M, how many milliliters (mL) of the NaOH solution is required to titrate the sulfuric acid present in the 10.0-mL portion of dilute acid solution? This acid-base reaction occurs as follows: H2SO4(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O(g) (A) 130. mL (B) 65.0 mL (C) 26.0 mL (D) 13.0 mL

We have to find volume of NaOH solution

Answered: how many milliliters (mL) of the NaOH…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions

Section: Chapter Questions

Problem 110IL: The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The...

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A 10.0-mL sample of sulfuric acid, H₂SO₄, from a battery of an old car is diluted to 100.0 mL, and a 10.00-mL aliquot (portion) of the diluted acid is then titrated with 0.2500 M NaOH solution. If the concentration of H₂SO₄ in the original battery was 3.25 M, how many milliliters (mL) of the NaOH solution is required to titrate the sulfuric acid present in the 10.0-mL portion of dilute acid solution? This acid-base reaction occurs as follows:

H₂SO₄(aq) + 2NaOH(aq) --> Na₂SO₄(aq) + 2H₂O(g)

(A) 130. mL

(B) 65.0 mL

(D) 13.0 mL

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